Chemical Elements.com - Zinc (Zn) Includes Zinc Facts and other information about the Element If you know of any other links for Zinc, please let me know Bentor, Yinon. Chemical Element.com - Zinc. < For more information about citing online sources, please visit the MLA's Website . This page was created by Yinon Bentor. Use of this web site is restricted by this site's license agreement . Copyright © 1996-2012 Yinon Bentor. All Rights Reserved. Zinc»the essentials [WebElements Periodic Table] CAS Registry ID : 7440-66-6 Zinc is a bluish-white, lustrous metal. It is brittle at ambient temperatures but is malleable at 100 to 150°C. It is a reasonable conductor of electricity, and burns in air at high red heat with evolution of white clouds of the oxide. The picture above shows the result from burning a mixture of zinc metal powder and sulphur (only to be demonstrated by a professionally qualified chemist). Zinc: historical information Zinc was discovered by Andreas Marggraf in 1746 at Germany. Origin of name : from the German word "zink".

Centuries before zinc was recognized as a distinct element, zinc ores were used for making brass (a mixture of copper and zinc). A brass dating from between 1400-1000 BC has been found in Palestine. An alloy containing 87% zinc was found in prehistoric ruins in Transylvania. The smelting of zinc ores with copper was apparently discovered in Cyprus and was used later by the Romans. Metallic zinc was produced in the 13th century in India by reducing calamine (zinc carbonate, ZnCO3) with organic substances such as wool. The metal was rediscovered later in Europe. William Champion set up a zinc industry in Bristol (England) in the 1740s. Other plants were established a little later in Belgium and Silesia. Sometime prior to the autumn of 1803, the Englishman John Dalton was able to explain the results of some of his studies by assuming that matter is composed of atoms and that all samples of any given compound consist of the same combination of these atoms.

Dalton also noted that in series of compounds, the ratios of the masses of the second element that combine with a given weight of the first element can be reduced to small whole numbers (the law of multiple proportions). This was further evidence for atoms. Dalton's theory of atoms was published by Thomas Thomson in the 3rd edition of his System of Chemistry in 1807 and in a paper about strontium oxalates published in the Philosophical Transactions. Dalton published these ideas himself in the following year in the New System of Chemical Philosophy. The symbol used by Dalton for zinc is shown below. [See History of Chemistry, Sir Edward Thorpe, volume 1, Watts & Co, London, 1914.] Zinc around us Read more » Zinc is essential in the diets of plants and animals. Zinc shortage in soils around the world is an important problem. Zinc is the key component of many enzymes. The protein hormone insulin contains zinc. Zinc plays a role in reproduction and also sexual maturation. Zinc deficiency resluts in stunted growth and in male sexual immaturity. This is reversed on the addition of zinc in the diet. Some organisms seem to accumulate zinc.

Zinc is never found as the free metal but there are a number of important ores such as sphalerite (zincblende, zinc sulphide, ZnS), smithsonite (zinc carbonate, ZnCO3), zincspar (also zinc carbonate, ZnCO3), and marmatite (zinc sulphide, ZnS, containing some iron sulphide, FeS). Zinc is wide spread around the world. Important deposits are located in North America and Australia. Abundances for zinc in a number of different environments. More abundance data » Location Second ionisation energy : 1733.3 kJ mol‑1 Isolation Isolation : zinc metal is readily available commercially so it is not normally necesary to make it in the laboratory. Most zinc production is based upon sulphide ores. These are roasted in industrial plants to form zinc oxide, ZnO. This may be reduced with carbon to form zinc metal, but in practice ingenious technology is required to ensure that the resulting zinc does not contain oxide impurities.

ZnO + C → Zn + CO ZnO + CO → Zn + CO2 CO2 + C → 2CO The other type of extraction is electrolytic. Dissolution of crude zinc oxide, ZnO, in sulphuric acid gives zinc sulphate, ZnSO4 in solution. Cadmium is an impurity and this is removed as a precipitate of cadmium sulphate by the addition of zinc dust. Electrolysis of the ZnSO4 solution using aluminium cathodes and lead alloyed with silver anodes gives pure zinc metal coated on the aluminium. Oxygen gas is liberated at the anode. Very pure zinc may be formed from crude zinc by zone refining and single crystals can be grown with purities of better than 99.9999%. Zinc isotopes Read more » Zinc isotopes are used extensively in both industrial and medical applications. Depleted Zn-64 is added to the cooling water of nuclear reactors in the form of oxide or acetate to prevent stress corrosion cracking. It also reduces the release of (stable) Co-59 into the cooling water by forming a thin spinel layer on the Co containing steel surfaces.

Neutron irradiation of Co-59 will result in the formation of Co-60, a radioisotope which emits high energy gamma radiation and is a major contributor to the dose rate of personnel working in the reactor. Enriched Zn-67 is often used in biological research into the uptake of Zn in the human body. It can also be used for the production of radioactive Ga-67 in smaller cyclotrons. However, by far most Ga-67 is made from Zn-68. Zn-67, Zn-68 and Zn-70 can all be used for the production of the therapeutic isotope Cu-67. Zn-66 has been proposed as an alternative target for the production of Cu-64 and Ga-67. Finally Zn-70 is also used in biological research and in research into super-heavy elements. Zinc - Element information, properties and uses | Periodic Table Chemistry in its element: zinc (Promo) You're listening to Chemistry in its element brought to you by Chemistry World, the magazine of the Royal Society of Chemistry.

(End promo) Chris Smith This week the chemical behind calamine lotion for itchy skin, anti dandruff shampoo for a flaky scalp and underarm deodorant for - well, I think we've probably all stood next to someone whom we wish knew a bit more about the chemistry of zinc. Here's Brian Clegg. Brian Clegg There aren't many elements with names that are onomatopoeic. Say 'oxygen' or 'iodine' and there is no clue in the sound of the word to the nature of the element. But zinc is different. Zinc - zinc - zinc - you can almost hear a set of coins falling into an old fashioned bath. It just has to be a hard metal. In use, Zinc is often hidden away, almost secretive. It stops iron rusting, soothes sunburn, keeps dandruff at bay, combines with copper to make a very familiar gold-coloured alloy and keeps us alive, but we hardly notice it. This blue-grey metal, known commercially as spelter, is anything but flashy and attention-grabbing. Even the origins of that evocative name are uncertain.

The dictionary tells us that the word zinc comes from the German (with a K at the end instead of a C), but how that name came into being is unknown. The earliest reference to zinc was in 1651. The substance was known before - objects with zinc in them date back over 2,500 years, and the Romans used that gold coloured alloy - but zinc wasn't identified as a distinct material in the west until the seventeenth century. Represented in the periodic table as Zn, zinc is a transition metal, grouped with cadmium and mercury. With the middling atomic number 30, it has five stable isotopes of atomic weight from the dominant zinc 64 to zinc 70, plus an extra 25 radioisotopes. Because of its hazy origins, it's difficult to pin down one person as the discoverer of the element. Although it seems to have been refined in India as early as the twelfth century, the earliest specific claim to have produced the metal was back in 1668, and a process for extracting zinc from its oxide was patented in the UK in 1738 by metal trader William Champion.

But it is usually the German chemist Andreas Marggraf who wins the laurels as 'discoverer' for his 1746 experiment isolating zinc. Although zinc's history is more than a little hazy, there's no doubting its usefulness. You've only got to look at a galvanized metal roof or bucket to see zinc at work. Galvanization is named after Luigi Galvani, the man who made frog legs twitch with electric current, but galvanization has nothing to do with electrical showmanship. In fact electricity's role is surprisingly subtle. The most common form of galvanization is hot dip galvanization, where iron or steel is slid through a bath of liquid zinc at around 460 degrees Celsius, forty degrees above its melting point. The coating prevents the object treated from rusting. Initially the zinc simply stops the air getting to the iron, but later the zinc corrodes in preference to iron in an electro-chemical process, acting as a so-called sacrificial anode. This is where the 'galvanic' part of the name comes in. Some galvanization is more literally electrical - car bodies, for example, are electroplated with zinc to apply a thin, even layer.

Zinc's electrical capabilities also extend to the most popular batteries. A traditional dry cell has an outer zinc casing acting as the anode (confusingly the anode, usually thought of as positive, is the negative end of a battery), while a carbon rod provides the cathode, the positive electrode. In the longer lasting alkaline batteries, the anode is formed from powdered zinc (giving more surface area for reaction), while the cathode is made up of the compound manganese dioxide. But the most visible example of zinc at work doesn't give any indication of this greyish metal - instead it's in an alloy that mixes the sheen of gold with the common touch. When molten zinc and copper are mixed together, the result is bold as brass. In fact, it is brass. Everything from door fixings to decorative plaques for horse collars have been made in this flexible alloy. Any orchestra would be much poorer without its brass instruments. It's even likely to turn up in the zips on your clothing. Well-polished brass has a pleasant glow - but our most intimate contact with zinc, or to be precise zinc oxide - often comes when dealing with the unwanted glow of sunburn.

When I was young and there was little in the way of sun block, sunburned skin would be lavishly coated in soothing pink calamine lotion. The primary ingredient of this is zinc oxide, which is white - it's small amounts of iron oxide that give it that colour. Even now, though, when we can avoid the need for calamine, zinc oxide plays its part. Called Chinese white when it's used in paints, zinc oxide is a good absorber of ultraviolet light - so sun block often contains a suspension of tiny zinc oxide particles - as does most mineral-based makeup. And that's just the start for this versatile oxide. You'll find it used in fire retardants and foods - where it fortifies the likes of breakfast cereals - in glass and ceramics, in glues and rubber. That surprise appearance on the breakfast table reflects another important side to zinc. We need it to stay healthy. It's one of the trace elements, nutrients that our bodies need in small quantities to keep functioning. It's often present in vitamin supplements, though most of us get plenty from meat and eggs. The zinc ends up in various proteins, particularly in enzymes involved in the development of the body, digestion and fertility.

A shortage of zinc in the diet can lead to delayed healing, skin irritation and loss of the sense of taste, and encourages many chronic illnesses. With zinc also appearing in anti-dandruff shampoos in the form of zinc pyrithione and in underarm deodorants as zinc chloride, this is an element that even makes us more attractive to the opposite sex. Zinc is a hidden star. We're rarely aware of it, unlike its flashier neighbours in the period table, but zinc is a workhorse element that helps us all. Chris Smith Bristolbased science writer Brian Clegg with the onomatopoeic element, zinc. Next week, what's lurking in your basement. Katherine Holt The first reports of problems associated with radon gas in domestic buildings was in the United States in 1984, when an employee at a nuclear power plant began setting off the radiation detector alarms on his way into work. The problem was eventually traced to his home, where the level of radon gas in the basement was found to be abnormally high. Chris Smith But where was it coming from and what was the risk to his health.

Katherine Holt will be here with all of the answers and the rest of the Radon story on next week's Chemistry in its Element, I do hope you can join us. I'm Chris Smith, thank you for listening, and goodbye. (Promo) Chemistry in its element is brought to you by the Royal Society of Chemistry and produced by thenakedscientists.com . There's more information and other episodes of Chemistry in its element on our website at chemistryworld.org/elements . (End promo) Zinc Facts - Periodic Table of the Elements Zinc Facts Zinc Facts Zinc Chemical & Physical Properties Zinc or spelter is a silvery-gray metallic element. This photo shows a cube of zinc, crystalline zinc from an ingot and sublimed dendritic zinc. Alchemist-hp Electron Configuration : [Ar] 4s2 3d10 Word Origin: German zinke: of obscure origin, probably German for tine. Zinc metal crystals are sharp and pointed. It could also be attributed to the German word 'zin' meaning tin. Isotopes: There are 30 known isotopes of zinc ranging from Zn-54 to Zn-83 .

Zinc has five stable isotopes: Zn-64 (48.63%), Zn-66 (27.90%), Zn-67 (4.10%), Zn-68 (18.75%) and Zn-70 (0.6%). Properties: Zinc has a melting point of 419.58°C, boiling point of 907°C, specific gravity of 7.133 (25°C), with a valence of 2. Zinc is a lustous blue-white metal. It is brittle at low temperatures, but becomes malleable at 100-150°C. It is a fair electrical conductor. Zinc burns in air at high red heat, evolving white clouds of zinc oxide. Uses: Zinc is used to form numerous alloys , including brass , bronze, nickel silver, soft solder, Geman silver, spring brass, and aluminum solder. continue reading below our video 4 Tips for Improving Test Performance Zinc is used to make die castings for use in the electrical, automotive, and hardware industries.

The alloy Prestal, consisting of 78% zinc and 22% aluminum, is nearly as strong as steel yet exhibits superplasticity. Zinc is used to galvanize other metals to prevent corrosion. Zinc oxide is used in paints, rubbers, cosmetics, plastics, inks, soap, batteries, pharmaceuticals, and many other products. Other zinc compounds are also widely used, such as zinc sulfide (luminous dials and fluorescent lights ) and ZrZn2 ( ferromagnetic materials ). Zinc is an essential element for humans and other animal nutrition. Zinc-deficient animals require 50% more food to gain the same weight as animals with sufficient zinc. Zinc metal is not considered toxic, but if fresh zinc oxide is inhaled it can cause a disorder referred to as zinc chills or oxide shakes. Sources: The primary ores of zinc are sphalerite or blende (zinc sulfide), smithsonite (zinc carbonate), calamine (zinc silicate), and franklinite (zinc, iron, and manganese oxides). An old method of producing zinc was by reducing calamine with charcoal.

More recently, it has been obtained by roasting the ores to form zinc oxide and then reducing the oxide with carbon or coal, followed by distillation of the metal. Zinc | Define Zinc at Dictionary.com zinc noun 1. Chemistry. a ductile, bluish-white metallic element: used in making galvanized iron, brass, and other alloys, and as an element in voltaic cells. Symbol: Zn; atomic weight: 65.37; atomic number: 30; specific gravity: 7.14 at 20°C. 2. a piece of this metal used as an element in a voltaic cell. verb (used with object), zincked or zinced [zingkt] /zɪŋkt/ (Show IPA), zincking or zincing [zing-king] /ˈzɪŋ kɪŋ/ (Show IPA) 3. to coat or cover with zinc.

Origin of zinc German 1635-1645 1635-45; < German Zink, perhaps derivative of Zinke(n) prong, tine, from the spikelike form it takes in a furnace Related forms Examples from the Web for zinc Expand Sally of Missouri R. E. Young In such a case, two, three, or more cells are connected so that the zinc of one is joined to the copper plate of the other. Physics Willis Eugene Tower British Dictionary definitions for zinc Expand noun 1. a brittle bluish-white metallic element that becomes coated with a corrosion-resistant layer in moist air and occurs chiefly in sphalerite and smithsonite. It is a constituent of several alloys, esp brass and nickel-silver, and is used in die-casting, galvanizing metals, and in battery electrodes. Symbol: Zn; atomic no: 30; atomic wt: 65.39; valency: 2; relative density: 7.133; melting pt: 419.58°C; boiling pt: 907°C 2.

C17: from German Zink, perhaps from Zinke prong, from its jagged appearance in the furnace Collins English Dictionary - Complete & Unabridged 2012 Digital Edition © William Collins Sons & Co. Ltd. 1979, 1986 © HarperCollins Publishers 1998, 2000, 2003, 2005, 2006, 2007, 2009, 2012 Word Origin and History for zinc Expand n. 1650s, from German Zink, perhaps related to Zinke "prong, point;" said to have been used first by Paracelsus (c.1526) on analogy of the form of its crystals after smelting. Zinke is from Old High German zint "a point, jag," from Proto-Germanic *tindja "tine" (cf. Old Norse tindr "point, top, summit," Old English tind "prong, spike;" cf. tine ).

Online Etymology Dictionary, © 2010 Douglas Harper Zinc - Elements Database Zinc Zinc Atomic Weight: 65.38 What is Zinc? Zinc (atomic number 30, symbol Z) is a chemical element and transition metal which is commonly found in the Earth's crust. This is a lustrous, reactive metal with a bluish-white color. It was discovered in 1746 by Andreas Marggraf, a German chemist who is known as a pioneer in the field of analytical chemistry. Isotopes and Chemical and Physical Properties Zinc is crystalline and brittle at normal temperatures and malleable and ductile at temperatures between 230 F (110 C) and 300 F (150 C). The element reacts with dilute acids and nonmetals. The melting point is 788 F (420 C) and the boiling point is 1664 F (907 C). Zinc combines with a number of elements, including tellurium, nickel, cobalt, magnesium, and tin. The metal also forms alloys with silver, lead, iron, gold, and bismuth.

Binary alloys are also formed when zinc reacts with antimony, aluminum, and copper. The element has a hexagonal packed structure and 10 isotopes. Zn-64 is the most abundant one. Occurrence The element is found in minerals such as hydrozincite, wurtzite, hemimorphite, smithsonite, and others. It occurs in soil, water, and air, and significant deposits are found in countries such as Iran, the U.S., Canada, and Australia. Commercial Uses and Applications This element has a number of commercial applications and is used to make different alloys. It alloys with magnesium, aluminum, and copper, and the alloys are used in the hardware, vehicle manufacturing, and other industries. It is alloyed with tin and lead to produce solder which is used for joining elements such as pipes and electrical components. American pennies are made using zinc in combination with other elements. Zinc also has applications in rubber manufacturing, inks, wallpaper and photocopier paper, cosmetics, and plastics. It is mainly used as a pigment. Zinc alloys have different applications and are commonly used for bending, roll forming, and deep drawing.

One of its compounds, zinc oxide is used in photocopying and varistors due to its good semiconductor properties. Zinc is also added to different mineral, vitamin, and other dietary supplements. It helps strengthen the immune response. Health and Environmental Effects Zinc is found in different foods, including wheat germ, lamb and beef, squash and pumpkin seeds, seafood, and spinach. It occurs free in nature and has antioxidant properties. High concentrations at waste sites increase the risk for health problems. Side effects include gastritis, diarrhea, vomiting, nausea, and other gastrointestinal problems. Other side effects are dyspepsia, stomachache, and unpleasant taste. High concentrations of zinc affect protein metabolism. It is a health hazard for newborn and unborn babies. Exposure occurs through breast milk and blood. At the same time, zinc is used to treat different illnesses and disorders, including anorexia nervosa, peptic ulcers, Hansen�s disease, Down syndrome, and Alzheimer�s disease. It is also used to treat Crohn�s disease, serious head injuries, tinnitus, and attention deficit-hyperactivity disorder. People at risk of zinc deficiency include lactating women, expectant mothers, vegetarians and vegans, and patients with gastrointestinal problems.

You can link to this page, using the code below: <a href="" title="Zinc - Periodic Table">Zinc - Periodic Table</a> Zinc, Chemical Element - reaction, uses, elements, examples, metal, gas, number, name PRONUNCIATION ZINK The most important use of zinc today is in galvanizing other metals. Galvanizing is the process of laying down a thin layer of zinc on the surface of a second metal. Zinc does not corrode (rust) as easily as iron and other metals. So the thin layer of zinc protects iron and other metals from corrosion. Discovery and naming Some metals can be obtained from their ores easily. In a few cases, all that is needed is to heat the ore. Heating an ore of zinc releases the free metal. But with zinc, there is an additional problem. Zinc metal sublimates very easily. Sublimation is the process by which a solid changes directly to a gas when heated, without first changing to a liquid. Anyone who wanted to make zinc from its ore would lose the zinc almost immediately by sublimation. Of course, early people did not understand this process. They may very well have made zinc by heating its ores.

But any zinc they made would have floated away immediately. Still, a process for extracting zinc from its ores was apparently invented in India by the 13th century. The process involves heating the zinc ore in a closed container. When zinc vapor forms, it condenses inside the container. It can then be scraped off and used. That method seems to have been passed to China and then, later, to Europe. In the meantime, ancient people were familiar with compounds and alloys of zinc. For example, there are brass objects from Palestine dating to 1300 B.C. Brass is an alloy of copper and zinc. The alloy may have been made by humans or found naturally in the earth. No one knows the origin of the brass in these objects. The first European to describe zinc was probably Swiss physician Paracelsus (1493-1541). Paracelsus' real name was Theophrastus Bombastus von Hohenheim. Early in life, he took the name Paracelsus, meaning "greater than Celsus." Celsus was one of the great Roman physicians.

Paracelsus wanted the world to know that he was even "greater than Celsus." Paracelsus was also an alchemist. Alchemy was a kind of pre-science that existed from about 500 B.C. to near the end of the 16th century. People who studied alchemy—alchemists—wanted to find a way to change lead, iron, and other metals into gold. They were also looking for the "secret to eternal life." Alchemy contained too much magic and mysticism to be a real science. But it developed a number of techniques and produced many new materials that were later found to be useful in modem chemistry. Paracelsus first wrote about zinc in the early 1500s. He described some properties of the metal. But he said he did not know what the metal was made of. Because of his report on the metal, Paracelsus is sometimes called the discoverer of zinc. The name zinc was first used in 1651. It comes from the German name for the element, Zink. What meaning that word originally had is not known. Physical properties Zinc is a bluish-white metal with a shiny surface.

It is neither ductile nor malleable at room temperature. Ductile means capable of being drawn into thin wires. Malleable means capable of being hammered into thin sheets. At temperatures above 100°C (212°F), however, zinc becomes somewhat malleable. Zinc's melting point is 419.5°C (787.1°F) and its boiling point is 908°C (1,670°F). Its density is 7.14 grams per cubic centimeter. Zinc is a fairly soft metal. Its hardness is 2.5 on the Mohs scale. The Mohs scale is a way of expressing the hardness of a material. It runs from 0 (for talc) to 10 (for diamond). Chemical properties Zinc is a fairly active element. It dissolves in both acids and alkalis. An alkali is a chemical with properties opposite those of an acid. Sodium hydroxide ("common lye") and limewater are examples of alkalis. Zinc does not react with oxygen in dry air. In moist air, however, it reacts to form zinc carbonate.

The zinc carbonate forms a thin white crust on the surface which prevents further reaction. Zinc burns in air with a bluish flame. Occurrence in nature The abundance of zinc in the Earth's crust is estimated to be about 0.02 percent. That places the element about number 24 on the list of the elements in terms of their abundance. A process for extracting zinc from its ores was apparently invented in India by the 13th century. Zinc never occurs as a free element in the earth. Some of its most important ores are smithsonite, or zinc spar or zinc carbonate (ZnCO 3 ); sphalerite, or zinc blende or zinc sulfide (ZnS); zincite, or zinc oxide (ZnO); willemite, or zinc silicate (ZnSiO 3 ); and franklinite [(Zn,Mn,Fe)O (Fe,Mn 2 )O 3 ]. The largest producer of zinc ore in the world today is Canada. Other important producing nations are Australia, China, Peru, the United States, and Mexico. In the United States, more than half of the zinc produced comes from Alaska.

Other important producing states are Tennessee, Missouri, Montana, and New York. Isotopes Five naturally occurring isotopes of zinc are known. They are zinc-64, zinc-66, zinc-67, zinc-68, and zinc-70. Isotopes are two or more forms of an element. Isotopes differ from each other according to their mass number. The number written to the right of the element's name is the mass number. The mass number represents the number of protons plus neutrons in the nucleus of an atom of the element. The number of protons determines the element, but the number of neutrons in the atom of any one element can vary. Each variation is an isotope. About eight radioactive isotopes of zinc are known also. A radioactive isotope is one that breaks apart and gives off some form of radiation. Radioactive isotopes are produced when very small particles are fired at atoms. These particles stick in the atoms and make them radioactive. One radioactive isotope of zinc, zinc-65, has some practical importance. Zinc-65 is used as a tracer to study physical and biological events. A tracer is an isotope whose presence in a system can easily be detected.

The isotope is injected into the system at some point. Inside the system, the isotope gives off radiation. That radiation can be followed by means of detectors placed around the system. Brass is an alloy of copper and zinc. For example, zinc-65 is used to study how alloys wear out. An alloy can be made using zinc metal. But the zinc used is zinc-65 instead of ordinary zinc. Changes in radiation given off by the radioactive isotope can be followed to find patterns in the way the alloy wears out. Zinc-65 can also be used to study the role of zinc in the human body. A person can be fed food that contains a small amount of zinc-65. The movement of the isotope through the body can be followed with a detector. A researcher can see where the isotope goes and what roles it plays in the body. Zinc oxide manufacturing. This compound is used to produce textiles, storage batteries, paints, and rubber products. Extraction As with many metals, pure zinc can be prepared from an ore by one of two methods. First, the ore can be roasted (heated in air).

Roasting converts the ore to a compound of zinc and oxygen, zinc oxide (ZnO). The compound can then be heated with charcoal (pure carbon ). The carbon takes the oxygen away from the zinc, leaving the pure metal behind: The other method is to pass an electric current through a compound of zinc. The electric current causes the compound to break apart. Pure zinc metal is produced. Zinc burns in air with a bluish flame. Uses The annual cost of corrosion (rusting) in the United States is estimated to be about $300 billion. This is money lost when metals become corroded and break apart. Buildings and The pipes of this beautiful church organ are made of zinc alloys. bridges are weakened, cars and trucks rust, farm equipment breaks down, and metal used in many other applications is destroyed. It is hardly surprising that protecting metal from corrosion is an important objective in American industry. One of the most effective ways of providing protection is through galvanizing. Today, about half of all the zinc produced in the United States is used to galvanize other metals. The largest consumers of galvanized metal are the construction and automotive industries. The second largest use of zinc is in making alloys.

An alloy is made by melting and mixing two or more metals. The mixture has properties different from those of the individual metals. Two of the most common alloys of zinc are brass and bronze. Brass is an alloy of zinc and copper. Bronze is an alloy of copper and tin that may also contain a small amount of zinc. Alloys of zinc are used in a great variety of products, including automobile parts, roofing, gutters, batteries, organ pipes, electrical fuses, type metal, household utensils, and building materials. Compounds A number of zinc compounds have important uses. Some examples are the following: Zinc deficiency can interfere with a plant's ability to reproduce.

zinc acetate (Zn(C 2 H 3 O 2 ) 2 ): wood preservative; dye for textiles; additive for animal feed; glazing for ceramics zinc arsenate (Zn 3 (AsO 4 ) 2 ): wood preservative; insecticide zinc borate (ZnB 4 O 7 ): fireproofing of textiles; prevents the growth of fungus and mildew zinc chloride (ZnCl 2 ): solder (for welding metals); fireproofing; food preservative; additive in antiseptics and deodorants; treatment of textiles; adhesives; dental cement; petroleum refining; and embalming and taxidermy products zinc fluorosilicate (ZnSiF 6 ): mothproofing agent; hardener for concrete zinc hydrosulfite (ZnS 2 O 4 ): bleaching agent for textiles, straw, vegetable oils, and other products; Zinc alloys are used in the production of electrical fuses.

brightening agent for paper and beet and cane sugar juice zinc oxide (ZnO): used in rubber production; white pigment in paint; prevents growth of molds on paints; manufacturer of glass; photocopy machines; production of many kinds of glass, ceramics, tile, and plastics zinc phosphide (Zn 3 P 2 ): rodenticide (rat killer) zinc sulfate (ZnSO 4 ): manufacture of rayon; supplement in animal feeds; dyeing of textiles; and wood preservative Health effects Zinc is an essential micronutrient for plants, humans, and animals. Zinc deficiency has relatively little effect on the health of a plant, but it interferes with reproduction. Pea plants deprived of zinc, for example, will form flowers. But the flowers will not turn to seeds. In humans, zinc deficiencies are more serious. Zinc is used to build molecules of DNA. DNA is the chemical in our body that tells cells what chemicals they should make. It directs the reproduction of humans also. Fetuses (babies that have not yet been born) deprived of zinc may grow up to have mental or physical problems. Young children who do not get enough zinc in their diet may experience loss of hair and skin lesions.

They may also experience retarded growth called dwarfism. Chemists have now found that zinc plays an essential role in the manufacture of many important chemicals in the human body. Zinc is an essential micronutrient for humans. But too much or too little can cause health problems. On the other hand, an excess of zinc can cause health problems, too. Breathing zinc dust may cause dryness in the throat, coughing, general weakness and aching, chills, fever, nausea, and vomiting. One sign of zinc poisoning is a sweet taste in the mouth that cannot be associated with eating sweet foods. Certain compounds of zinc can be harmful to health also. Zinc chloride (ZnCl 2 ), for example, can cause skin rashes and sore throat. User Contributions: Zinc Mineral Data Electron Density: Bulk Density (Electron Density)=6.60 gm/cc note: Specific Gravity of Zinc =7.19 gm/cc. Fermion Index: Fermion Index = 0.04 Boson Index = 0.96 U=PEZinc x rElectron Density= 342.72 barns/cc.

Radioactivity: GRapi = 0 (Gamma Ray American Petroleum Institute Units) Zinc is Not Radioactive Zinc Classification Dana Class: 01.01.05.01 (01) Native Elements (01.01) with metallic elements other than the platinum group (01.01.05) Dana Group 01.01.05.01 Zinc Zn P 63/mmc 6/m 2/m 2/m 01.01.05.02 Cadmium Cd P 63/mmc 6/m 2/m 2/m Strunz Class: 01.AB.05 01 - ELEMENTS (Metals and intermetallic alloys; metalloids and nonmetals; carbides, silicides, nitrides, phosphides) 01.A - Metals and Intermetallic Alloys 01.AB -Zinc-brass family (Cu-Zn alloys) 01.AB.05 Cadmium Cd P 63/mmc 6/m 2/m 2/m zinc acetate | C4H6O4Zn | ChemSpider zinc acetate CC(=O

)[O-].CC(=O)[O- ].[Zn+2] CSID:10719, (accessed 22:18, Jan 19, 2017) Copy Diacétate de zinc [French] [ACD/IUPAC Name] Zinc di(acetate) Validated by Experts, Validated by Users, Non-Validated, Removed by Users 383317_ALDRICH [DBID] 200 °C (Decomposes) Alfa Aesar 200 °C (Decomposes) Alfa Aesar 35792 , H33734 83-86 °C LabNetwork LN00222346 1.84 g/mL Alfa Aesar 35792 1.84 g/l Fluorochem 494138

Question: What is the chemical symbol for Zinc?
Answer: ZN